SCIENCE UNDERSTANDING Different types of chemical reactions are used to produce a range of products and can occur at different rates. (4-6 lessons)
NAME:
Science Quest TEXTBOOK
SCIENCE Quest PRACTICALS / ACTIVITIES
SCIENCE Quest HOMEWORK
OTHER ACTIVITIES/RESOURCES
1
5.1 – A Game of Balance – Develop an understanding of the translation of word equations to symbols in the writing of balanced chemical equations.
Activities in the section p.162 – 164) - Game Rules - Play the Game. Checking for Balance interactivity int-0677 ebook
Questions from textbook p. 164 Qn’s – 1 -3 Worksheet 5.1 – Chemical Equations Worksheet 5.2 – Balancing Chemical Equations Worksheet 5.3 - A World of Reactions
5.2 –Precipitation Reactions – Develop an understanding of equation writing by completing activities related to precipitation reactions - Utilise solubility table given on p. 165 to develop students’ understanding of soluble/ insoluble compounds formed and the precipitation reactions related to these precipitates.
Suggestions: Investigation 5.2 – Will it Precipitate p.166 Qn’s 1 - 5
Questions from textbook p. 166 – Qn’s 1 – 6 Worksheet 5.4 Precipitation
Words to Learn - ionic compounds, precipitate, precipitation reactions
3
5.3 – Chemicals can be a Health Hazard – Describe the dangers associated with each of the classes and subclasses of substances classified as dangerous goods. Have students have an awareness of more common chemical symbols encountered.
Read and complete section and p.169 Qn’s 1-6
Words to Learn - terms used on dangerous goods symbols
4
5.4 – A World of Reactions – students to have an awareness of combustion reactions hydrocarbons + oxygen carbon dioxide + water
Take appropriate notes
examples of balanced combustion rxtns
5
5.7 –Rates of Reaction– Describe the role of catalysts in a chemical reaction and investigate the use of naturally occurring catalysts in the human body.
Investigation 5.4 – A Liver Catalyst
Read and complete section and textbook questions p. 184 – Qn’s 1-5 Worksheet 5.4 p. 184 - A Liver Catalyst
Words to Learn - rate, catalyst, enzyme
6
Assessment – completion of 2 practical reports (as above) - assessment of concepts from relevant exam questions on the Mid Year Exam
The law of conservation of matter (mass)This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction. They may have combined differnetly and have formed another compound or they may change state.
In an experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was 205g
The mass after the reaction was _205g__(some student's did not get teh same mass eg 1 group got 204.6g
Why were their masses different? They should not be different. It was expected to be the same. Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How does this relates to equations of reactions?
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2 This is an example of a carbonate plus an acid reactionBig number at the front of a element or compound means to multiply all the elements in the compound by that number.
A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions neutralisation reactions
This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water
General form: Acid + Base -----> Salt + Water
Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water
HCl + NaOH -------> NaCl + H2O
Examples of acids:hydrochloric acid HCl
Sulfuric acid H2SO4
Nitric acid HNO3
Vinegar or Citric acid CH3COOH
Examples of basesSodium Hydroxide NaOH
Calcium Hydroxide Ca(OH)2
Magnesium Hydroxide Mg(OH)2
metal hydroxide
Practice
Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first]
,Write equations for
Mg(OH)2 +H2SO4
Mg(OH)2 +HNO3
NaOH + H2SO4
Combustion ReactionsCombustion reactions is when oxygen is combined with another compound or element. We call this combining burning.
Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O Precipitationsolution + solution ----> solid + solution Its important to realise that the product of a precipitation reaction is a coloured solid that makes the solution change from a see through solution to an opaque solution. The subscripts s aq l and g are requiredegPb(NO3)2(aq) + KI(aq) --------->PbI2 (s) +2KNO3(aq)
Rates of ReactionWe know a reaction has occured if bubbles of gas are produced, a colour change happens or a temperature change occurs.How fast this happens is called the rate of a reaction. Eg rusting is a very slow combustion reaction. Propane gas burning to heat the BBQ is a very fast reaction.Rate refers to how fast the reaction reaches completion. The expt with liver and peroxide showed that
peroxide by itself gave off very few bubbles
peroxide with a lump of liver gave off quite a few bubbles
peroxide and finely chopped liver gave off lots of bubbles.
In this expt the liver was the catalyst. we increased the rate of the reaction by adding the catalyst. The definition of a catalyst is " a chemical that speeds up a reaction but does not become part of the products in the reactions.We increase the effectiveness of the catalyst by chopping it up - this increased the surface area on which the reaction can take place.
This expt increases the rate by increasing the concentration and the temperature of the reactants.The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How would we test this?To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate.
The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
How Does Temperature affect the reaction rateIncrease in temp leads to increase in reaction rate.This is because an increase in temperature will increase the kinetic energy of the particles in the reaction making them move faster and bump into more particle sand so more chances of reacting hence the reaction rate is faster. Biologicalcatalysts
Enzymes are biological catalysts. They speed up rxtns .
Eg digestion of starch involves amylase. Amylase is the enzyme. It speeds up the reactns to break down starch into simple sugars.
Summaryreaction rate is increased if
temperature is increase
concentration of reactants is increase
surface area is increase
use of a catalyst
Carbon ChemistryCarbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.
The simplest organic chemicals are the hydrocarbons.
Hydrocarbons with single bonds between the Carbons are called ALKANES.
Hydrocarbons with a double bond between one of the carbons are called ALKENES
Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol
This is the old course Name
Key Concept
Vocabulary
Common Assessment Tasks
Patterns, order and organization
Form and function
Stability and change
Systems
Different types of chemical reactions are used to produce a range of products and can occur at different rates
Qn 7 p. 201 Checking for balance interactivity. int-0677
5.1 Chemical equations 5.2 Balancing chemical equations 5.3 A world of reactions
Weblink
Use the Balancing equations weblink in the eBookPLUS to learn more about balancing chemical equations
Extension
Qn 11 – Imagine – Creative Writing Activity
Qn 12 – Investigate – Practical Design Activity
__
Weeks 2-3
Different types of Reactions 5.3 Precipitation Reactions 5.4 A World of Reactions - Discuss combustion, breaking down and combination reactions 5.5 The Need for Speed – Discuss catalysts
More ground work on balancing equations a table of valencies
balancing work sheet 1 Activity: Ionic formulas sheet
Use the Introduction to reactions weblink in your eBookPLUS to find out more about precipitation and other reactions.
Inquiry Investigation 5.2 - Will it precipitate?
p. 203 5.4 Precipitation
Inquiry Investigation 5.3- Decomposing powder p. 203
Inquiry Investigation 5.5- A Liver Catalyst p.220
Answer Questions 1 – 3 p. 220
5.5 Chemicals can be a Health Hazard Qn’s 1-7
Week 4
5.6 Fuelling our Lifestyle Science as a human endeavor - Discuss fuel sources - fossil fuels, fractional distillation, biofuels, biomass, biogas, ethanol
Answer Questions 1-10 p. 217
Qn 15 p. 217
Week 5
END OF TOPIC TEST
STUDY FOR SEMESTER TWO EXAMS
Class Notes
The law of conservation of matter (mass)
This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction.
In an experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was
The mass after the reaction was ___the same
Why were the masses different? They should not be different
It was expected to be the same. Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How this relates to equations of reactions.
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2 This is an example of a carbonate plus an acid reaction
Big number at the front of a element or compound means to multiply all the elements in the compound by that number.
A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions neutralisation reactions
This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water
General form: Acid + Base -----> Salt + Water
Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water
HCl + NaOH -------> NaCl + H2O
Practice
Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first]
,Write equations for
Mg(OH)2 +H2SO4
Mg(OH)2 +HNO3
NaOH + H2SO4
Combustion Reactions
Combustion reactions is when oxygen is combined with another compound or element. We call this combining burning.
Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O
Precipitation
solution + solution ----> solid + solution
Rates of Reaction
Rate refers to the how fast the reaction reaches completion. The expt with liver and peroxide showed that
peroxide by itself gave off very few bubbles
peroxide with a lump of liver gave off quite a few bubbles
peroxide and finely chopped liver gave off lots of bubbles.
In this expt the liver was the catalyst. we increased the rate of the reaction by adding the catalyst. The definitioin of a catalyst is " a chemical that speeds up a reaction but does not become part of thte products in the reactions. We increase the effectiveness of the catalyst by chopping it up - this increased the surface area on which the reaction can take place. This expt increases the rate by increasing the concentration and the temperature of the reactants. The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How would we test this?To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate.
The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
How Does Temperature affect the reaction rateIncrease in temp leads to increase in reaction rate.This is because an increase in temperature will increase the kinetic energy of the particles in the reaction making them move faster and bump into more particle sand so more chances of reacting hence the reaction rate is faster. Summary reaction rate is increased if
temperature is increase
concentration of reactants is increase
surface area is increase
use of a catalyst
Carbon Chemistry
Carbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.
The simplest organic chemicals are the hydrocarbons.
Hydrocarbons with single bonds between the Carbons are called ALKANES.
Hydrocarbons with a double bond between one of the carbons are called ALKENES
Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol
The properties and structure of materials in terms of their constituent particles and forces holding them together.
Construct and use atomic symbols and balanced equations to summarise chemical equations eg; neutralization, precipitation and combustion.
The sustainable management of a resource.
Chemical change in terms of energy.
mixtures compounds elements solutions solvent solute bonding: ionic, metallic, covalent physical and chemical change reactants and products conservation of matter rate of reaction
catalyst yield enzymes formula hydrocarbons homologous alkanes alkenes alkynes functional group
combustion neutralisation precipitation biodegradable pressure temperature molecule atom electron proton anion/cation
Practical write up – student choice from pracs listed in suggested activities Research report – student choice from research listed in extension & variation Test
Done @ School Teacher Signs
Done @ Home Teacher signs
Priority 1
Suggested Activities
Extension and Variation
2.1: Matter – Revision - (very fast) states of matter, elements, compounds, mixtures, solutions. Bonding – metallic, ionic and covalent (review fast) Physical and chemical change (review fast) Conservation of mass (review fast) Balancing and writing Chemical equations (review fast) Types of Reactions: neutralisation, combustion and precipitation
Questions: 1-4 (p56), sheet Prac: Study of a reaction (p58) Activity: Ionic formulas sheet
Prac: Precipitation Reactions (sheet) Homework Book: 2.2 Chem and Phys Change (p18-19)(DIM BK3) Prac: Conservation of mass (p58) Questions: 10-13(p56) Homework Book: 2.3 Classifying reaction types (p20) (DIM BK3)/ 2.2 Revising chemical equations (p26) Homework Book: 2.3 and 2.4 (p28-31) Online test for valency Access Key is 8C7F remember to type your class in front of your first name
Balancing more equations
It would help you to write out these equations as you work out the answers.
Investigate: Find out more about ionic, metallic and covalent bonding (p57) Questions: More balancing equations (sheet) Science at Work: Maths in Chemistry (p59) Balancing equations 4 worksheets with answers.
2.2 Rate and Yield – investigating how experimental conditions affect how fast a reaction proceeds and how much products are made
Prac: calculating the rate of reaction (p69) Questions: 1-3 (p67) Prac: Effect of concentration, surface area, temp and catalyst on reaction rate (exps p 70-71) Questions: 4-13 (p68) Research Assignment: The commercial production of a chemical of importance. Homework: 2.7 rates of reaction (p.38- 39)
Surfing: Companion website – assessing risk(p68) Research: how do air bags work (p.69)
2.3 Organic Chemistry – investigating the properties, types and reactions of compounds classified as organic. (alkanes, alkenes, and alcohols)
Investigate: Types of organic compounds and their bonding (p.72-75) - name and draw alkanes (methane to decane) name and draw alkenes (ethene to pentene) name and draw alcohols (methanol to butanol) Prac: Making barrier cream (sheet) Questions: 2-15 ( p77) Homework Book: 2.8 Organic Chemistry (p.40)
Surfing: Companion website: find the role of bubble caps in fractional distillation (p.78) Research: Different types of everyday Organic Chemicals
2.4: Green Chemistry – understanding the environmental concerns related to the commercial production of chemicals. Revision Test
Investigate: The principles of Green Chemistry Questions: 1-14 (p.82) Prac: Exploring the biodegradability of plastic (p.83)
Surfing: The history of Green Chemistry (p.83) Analysing: Find a media article on a biodegradable product (p.83)
Revision and test preparation
Text Book: Chapter review p 84 questions 1 to 20
Revision sheet - bring your laptops to complete the online component of the test.
This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction.
In our experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was The mass after the reaction was ___
Why were the masses different?
It was expected to be the same. Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How this relates to equations of reactions.
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2 This is an example of a carbonate plus an acid reaction
Big number at the front of a element or compound means to multiply all the elements in the compound by that number.
A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions neutralisation reactions This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water General form: Acid + Base -----> Salt + Water Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water HCl + NaOH -------> NaCl + H2O
Practice Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first] ,Write equations for
Mg(OH)2 +H2SO4
Mg(OH)2 +HNO3
NaOH + H2SO4
Combustion Reactions
Combustion reactions is when oxygen is combined with another compound or element. We call this combining burning.
Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O
Precipitation
solution + solution ----> solid + solution
Rates of Reaction
Rate refers to the how fast the reaction reaches completion. The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.
This expt showed the effect of concentration on the rate of the reaction. Paste your graph you made using excel into your notes. In conclusion the higher the concentration the ___ the reaction.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How did we test this? To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate. The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
Does Temperature affect the reaction rate? Describe the way we tested this question- list your ideas in point form. 1. we measured the temp of the sodium thiosulfate 2. added the acid and timed until the cross disappeared 3. we repeated steps 1 and 2 but we increased the temp of the sodium thiosulphate by sitting it in a water bath until its temp increased 10C from the time before 4. we did this 4 times.
Graph these results
Temp deg C
Time in Seconds
15
33
25
13
35
6
45
4
The reason the reaction was faster is because hotter the chemicals the faster the particles move. When particles are moving fast they are more likely to hit each other. Hence they will react.
Rates of reaction and catalysts
A catalyst is a chemical that can speed up a reaction but is not used up in the reaction Expt Prac 5 P 71 Aim: To describe the effect of a catalyst Method 1. 10 Ml of H2O2 (hydrogen peroxide) in beaker A and in beaker B - Beaker A will be the control 2. Add small amount of Manganese dioxide MnO2 to beaker B- record observations 3. To Beaker C Add 10Mls of H2O2 and then Add 5 drops of NaOH and 10 Drops of KI-
Results Observation Beaker A small bubbles of oxygen Beaker B lots of bubbles of oxygen- vigorous reaction Beaker C cancelled Conclusion Manganese dioxide was a catalyst that made the reaction rate increase (more bubbles) but did not seem to change itself- it was still a black powder.
Carbon Chemistry
Carbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.
The simplest organic chemicals are the hydrocarbons. Hydrocarbons with single bonds between the Carbons are called ALKANES. Hydrocarbons with a double bond between one of the carbons are called ALKENES Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol
Year 10 Science - Chemical Reactions– Outline
2015 Year 10 Chemical Reactions
Different types of chemical reactions are used to produce a range of products and can occur at different rates. (4-6 lessons)
TEXTBOOK
HOMEWORK
- Game Rules
- Play the Game.
Checking for Balance interactivity int-0677 ebook
Worksheet 5.1 – Chemical Equations
Worksheet 5.2 – Balancing Chemical Equations
Worksheet 5.3 - A World of Reactions
https://www.educationperfect.com/login/#Task=84248
Go here for a Valency table and a step by step process of how to balance equations. Courtesy of Mr Warden.
Also a good animation and simulation on how balancing really works from Colorado Uni
Activity: Ionic formulas sheet
- chemical equations
- Utilise solubility table given on p. 165 to develop students’ understanding of soluble/ insoluble compounds formed and the precipitation reactions related to these precipitates.
Investigation 5.2 – Will it Precipitate p.166 Qn’s 1 - 5
Worksheet 5.4 Precipitation
- ionic compounds, precipitate, precipitation reactions
Describe the dangers associated with each of the classes and subclasses of substances classified as dangerous goods. Have students have an awareness of more common chemical symbols encountered.
- terms used on dangerous goods symbols
Worksheet 5.4 p. 184 - A Liver Catalyst
- rate, catalyst, enzyme
- assessment of concepts from relevant exam questions on the Mid Year Exam
8C7F remember to type your class in front of your first name
Class notes
Class Notes
The law of conservation of matter (mass)This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction. They may have combined differnetly and have formed another compound or they may change state.In an experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was 205g
The mass after the reaction was _205g__(some student's did not get teh same mass eg 1 group got 204.6g
Why were their masses different? They should not be different. It was expected to be the same.
Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How does this relates to equations of reactions?
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2
This is an example of a carbonate plus an acid reactionBig number at the front of a element or compound means to multiply all the elements in the compound by that number.
A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions
neutralisation reactions
This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water
General form: Acid + Base -----> Salt + Water
Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water
HCl + NaOH -------> NaCl + H2O
Examples of acids:hydrochloric acid HCl
Sulfuric acid H2SO4
Nitric acid HNO3
Vinegar or Citric acid CH3COOH
Examples of basesSodium Hydroxide NaOH
Calcium Hydroxide Ca(OH)2
Magnesium Hydroxide Mg(OH)2
metal hydroxide
Practice
Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first]
,Write equations for
Combustion ReactionsCombustion reactions is when oxygen is combined with another compound or element. We call this combining burning.
Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O
Precipitationsolution + solution ----> solid + solution Its important to realise that the product of a precipitation reaction is a coloured solid that makes the solution change from a see through solution to an opaque solution. The subscripts s aq l and g are requiredegPb(NO3)2(aq) + KI(aq) --------->PbI2 (s) +2KNO3(aq)
Rates of ReactionWe know a reaction has occured if bubbles of gas are produced, a colour change happens or a temperature change occurs.How fast this happens is called the rate of a reaction. Eg rusting is a very slow combustion reaction. Propane gas burning to heat the BBQ is a very fast reaction.Rate refers to how fast the reaction reaches completion. The expt with liver and peroxide showed that
In this expt the liver was the catalyst. we increased the rate of the reaction by adding the catalyst. The definition of a catalyst is " a chemical that speeds up a reaction but does not become part of the products in the reactions.We increase the effectiveness of the catalyst by chopping it up - this increased the surface area on which the reaction can take place.
This expt increases the rate by increasing the concentration and the temperature of the reactants.The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How would we test this?To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate.
The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
How Does Temperature affect the reaction rateIncrease in temp leads to increase in reaction rate.This is because an increase in temperature will increase the kinetic energy of the particles in the reaction making them move faster and bump into more particle sand so more chances of reacting hence the reaction rate is faster.
Biological catalysts
Enzymes are biological catalysts. They speed up rxtns .
Eg digestion of starch involves amylase. Amylase is the enzyme. It speeds up the reactns to break down starch into simple sugars.
Summaryreaction rate is increased if
Carbon ChemistryCarbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.
The simplest organic chemicals are the hydrocarbons.
Hydrocarbons with single bonds between the Carbons are called ALKANES.
Hydrocarbons with a double bond between one of the carbons are called ALKENES
Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol
This is the old course
Name
Different types of chemical reactions are used to produce a range of products and can occur at different rates
plastic
polymer
polymerisation
monomer
copolymer
crosslinks
thermosetting polymer thermoplastic polymers
precipitation
aqueous solution
combustion reactions
hydrocarbons
decomposition reactions
combination reactions
fossil fuels
fractional distillation biofuels
biomass
biogas
ethanol
catalyst
- Different types of polymers – definition of monomers, polymers, copolymers, thermosetting and thermoplastic polymers
5.2 A Game of Balance p. 199 – balancing Equations__
5.1 Chemical equations
5.2 Balancing chemical equations
5.3 A world of reactions
- Weblink
Use the Balancing equations weblink in the eBookPLUS to learn more about balancing chemical equations- Qn 11 – Imagine – Creative Writing Activity
- Qn 12 – Investigate – Practical Design Activity
__2-3
5.3 Precipitation Reactions
5.4 A World of Reactions
- Discuss combustion, breaking down and combination reactions
5.5 The Need for Speed
– Discuss catalysts
More ground work on balancing equations
a table of valencies
balancing work sheet 1
Activity: Ionic formulas sheet
Homework Book: 2.1 Writing Formulas (p24-25)/2.1 Ionic compounds p16-17 (DIM BK3)
Go here for a Valency table and a step by step process of how to balance equations. Courtesy of Mr Warden.
Also a good animation and simulation on how balancing really works from Colorado Uni
- Weblink
Use the Introduction to reactions weblink in your eBookPLUS to find out more about precipitation and other reactions.- Inquiry Investigation 5.2 - Will it precipitate?
p. 203- Inquiry Investigation 5.3- Decomposing powder p. 203
- Inquiry Investigation 5.5- A Liver Catalyst p.220
Answer Questions 1 – 3 p. 220Qn’s 1-7
Science as a human endeavor
- Discuss fuel sources - fossil fuels, fractional distillation, biofuels, biomass, biogas, ethanol
STUDY FOR SEMESTER TWO EXAMS
Class Notes
The law of conservation of matter (mass)
This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction.In an experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was
The mass after the reaction was ___the same
Why were the masses different? They should not be different
It was expected to be the same. Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How this relates to equations of reactions.
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2 This is an example of a carbonate plus an acid reaction
Big number at the front of a element or compound means to multiply all the elements in the compound by that number.A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions
neutralisation reactions
This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water
General form: Acid + Base -----> Salt + Water
Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water
HCl + NaOH -------> NaCl + H2O
Examples of acids:
hydrochloric acid HClSulfuric acid H2SO4
Nitric acid HNO3
Vinegar or Citric acid CH3COOH
Examples of bases
Sodium Hydroxide NaOHCalcium Hydroxide Ca(OH)2
Magnesium Hydroxide Mg(OH)2
metal hydroxide
Practice
Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first]
,Write equations for
Combustion Reactions
Combustion reactions is when oxygen is combined with another compound or element. We call this combining burning.Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O
Precipitation
solution + solution ----> solid + solutionRates of Reaction
Rate refers to the how fast the reaction reaches completion. The expt with liver and peroxide showed thatIn this expt the liver was the catalyst. we increased the rate of the reaction by adding the catalyst. The definitioin of a catalyst is " a chemical that speeds up a reaction but does not become part of thte products in the reactions.
We increase the effectiveness of the catalyst by chopping it up - this increased the surface area on which the reaction can take place.
This expt increases the rate by increasing the concentration and the temperature of the reactants.
The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How would we test this?To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate.
The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
How Does Temperature affect the reaction rateIncrease in temp leads to increase in reaction rate.This is because an increase in temperature will increase the kinetic energy of the particles in the reaction making them move faster and bump into more particle sand so more chances of reacting hence the reaction rate is faster.
Summary
reaction rate is increased if
Carbon Chemistry
Carbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.The simplest organic chemicals are the hydrocarbons.
Hydrocarbons with single bonds between the Carbons are called ALKANES.
Hydrocarbons with a double bond between one of the carbons are called ALKENES
Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol
-------------------------------------------------------------------------------------------
0ld course
Chemical Reactions -key concepts – student guide 4 weeks duration Name__
Online component of the test
compounds
elements
solutions
solvent
solute
bonding: ionic, metallic, covalent
physical and chemical change
reactants and products
conservation of matter
rate of reaction
yield
enzymes
formula
hydrocarbons
homologous
alkanes
alkenes
alkynes
functional group
neutralisation
precipitation
biodegradable
pressure
temperature
molecule
atom
electron
proton
anion/cation
Research report – student choice from research listed in extension & variation
Test
Teacher Signs
Teacher signs
Bonding – metallic, ionic and covalent (review fast)
Physical and chemical change (review fast)
Conservation of mass (review fast)
Balancing and writing Chemical equations (review fast)
Types of Reactions: neutralisation, combustion and precipitation
Prac: Study of a reaction (p58)
Activity: Ionic formulas sheet
Homework Book: 2.1 Writing Formulas (p24-25)/2.1 Ionic compounds p16-17 (DIM BK3)
Go here for a Valency table and a step by step process of how to balance equations. Courtesy of Mr Warden.
Also a good animation and simulation on how balancing really works from Colorado Uni
Prac: Precipitation Reactions (sheet)
Homework Book: 2.2 Chem and Phys Change (p18-19)(DIM BK3)
Prac: Conservation of mass (p58)
Questions: 10-13(p56)
Homework Book: 2.3 Classifying reaction types (p20) (DIM BK3)/
2.2 Revising chemical equations (p26)
Homework Book: 2.3 and 2.4 (p28-31)
Online test for valency Access Key is
8C7F remember to type your class in front of your first name
Balancing more equations
It would help you to write out these equations as you work out the answers.
Practice balancing equations - here is a game where you fill in the blanks
http://www.sciencegeek.net/Chemistry/taters/EquationBalancing.htm
Here is another game to play balancing the equations
http://www.files.chem.vt.edu/RVGS/ACT/notes/scripts/bal_eq1.html
This one is a bit harder - read the instructions carefully - it would help you to write out the equation as you do these
http://www.syvum.com/cgi/online/fillin.cgi/squizzes/chem/baleq1.tdf?0
Questions: More balancing equations (sheet)
Science at Work: Maths in Chemistry (p59)
Balancing equations 4 worksheets with answers.
Questions: 1-3 (p67)
Prac: Effect of concentration, surface area, temp and catalyst on reaction rate (exps p 70-71)
Questions: 4-13 (p68)
Research Assignment: The commercial production of a chemical of importance.
Homework: 2.7 rates of reaction (p.38- 39)
Research: how do air bags work (p.69)
(alkanes, alkenes, and alcohols)
name and draw alkenes (ethene to pentene)
name and draw alcohols (methanol to butanol)
Prac: Making barrier cream (sheet)
Questions: 2-15 ( p77)
Homework Book: 2.8 Organic Chemistry (p.40)
Research: Different types of everyday Organic Chemicals
Revision
Test
Questions: 1-14 (p.82)
Prac: Exploring the biodegradability of plastic (p.83)
Analysing: Find a media article on a biodegradable product (p.83)
Revision sheet - bring your laptops to complete the online component of the test.
Class Notes
The law of conservation of matter (mass)
This states that matter can not be created nor destroyed. In chemistry this means that when we observe a reaction the elements present at the start of the reaction will also be present at the end of the reaction.In our experiment we added calcium carbonate to hydrochloric acid in a closed conical flask while it sat on an electronic balance.
We knew a reaction happened because we saw - bubbles, balloons full of gas and the marble chip (calcium carbonate) got smaller.
The mass at the beginning of the reaction was
The mass after the reaction was ___
Why were the masses different?
It was expected to be the same. Any difference may be due to the electronic balance being left on for a long period of time and losing accuracy.
How this relates to equations of reactions.
The elements in the reactants should be in the same quantity in the product.
This means if our equation shows 1 calcium atom on the reactant side it should have one calcium on the product side. If it does not we have to go through a process called balancing the equations.
The reaction for this experiment is
CaCO3 + 2 HCl ----> CaCl2 + H2O + CO2 This is an example of a carbonate plus an acid reaction
Big number at the front of a element or compound means to multiply all the elements in the compound by that number.A little number behind a letter means you multiply that letter (element) by that number to work out how many atoms of that element are in the reaction.
For more information on how to balance equations go here AND GO HERE FOR AN ANIMATION
Types of reactions
neutralisation reactions
This is when an acid is added to a base. These two compounds neutralise each other and form a salt and water
General form: Acid + Base -----> Salt + Water
Example; Hydrochloric acid + sodium hydroxide -------> sodium chloride + water
HCl + NaOH -------> NaCl + H2O
Examples of acids:
hydrochloric acid HClSulfuric acid H2SO4
Nitric acid HNO3
Vinegar or Citric acid CH3COOH
Examples of bases
Sodium Hydroxide NaOHCalcium Hydroxide Ca(OH)2
Magnesium Hydroxide Mg(OH)2
metal hydroxide
Practice
Write a balanced equation for sodium hydroxide + Nitric Acid [Hint write the word equation first]
,Write equations for
Combustion Reactions
Combustion reactions is when oxygen is combined with another compound or element. We call this combining burning.Common example is methane + oxygen ------> Carbon dioxide + water
CH 4 + O2 ----> CO2 + H2O
Precipitation
solution + solution ----> solid + solutionRates of Reaction
Rate refers to the how fast the reaction reaches completion. The expt with the sodium thiosulphate and hydrochloric acid reached completion when all the liquid turned a milky yellow.This expt showed the effect of concentration on the rate of the reaction.
Paste your graph you made using excel into your notes.
In conclusion the higher the concentration the ___ the reaction.
Size of the particles in a reaction affects the surface area that is exposed to react. For example 10g of calcium carbonate crushed as powder will result in very small particles. These will have a larger surface area when compared to a 10g stone of calcium carbonate (marble)
How did we test this?
To ensure it was a fair test we USed same amount of acid and the same mass of calcium carbonate.
The powder was faster because - it has the largest surface area - it would spread out over the desk the furthest. The rock would not spread out.
Does Temperature affect the reaction rate?
Describe the way we tested this question- list your ideas in point form.
1. we measured the temp of the sodium thiosulfate
2. added the acid and timed until the cross disappeared
3. we repeated steps 1 and 2 but we increased the temp of the sodium thiosulphate by sitting it in a water bath until its temp increased 10C from the time before
4. we did this 4 times.
Graph these results
The reason the reaction was faster is because hotter the chemicals the faster the particles move. When particles are moving fast they are more likely to hit each other. Hence they will react.
Rates of reaction and catalysts
A catalyst is a chemical that can speed up a reaction but is not used up in the reactionExpt
Prac 5 P 71
Aim: To describe the effect of a catalyst
Method
1. 10 Ml of H2O2 (hydrogen peroxide) in beaker A and in beaker B - Beaker A will be the control
2. Add small amount of Manganese dioxide MnO2 to beaker B- record observations
3. To Beaker C Add 10Mls of H2O2 and then Add 5 drops of NaOH and 10 Drops of KI-
Results
Observation
Beaker A small bubbles of oxygen
Beaker B lots of bubbles of oxygen- vigorous reaction
Beaker C cancelled
Conclusion Manganese dioxide was a catalyst that made the reaction rate increase (more bubbles) but did not seem to change itself- it was still a black powder.
Carbon Chemistry
Carbon chemistry's other name is organic chemistry. It is chemistry of living things and as such it usually only involves the elements - Carbon, Hydrogen and Oxygen ( Nitrogen too in some cases). This means water is an organic compound as is Natural gas - Methane.The simplest organic chemicals are the hydrocarbons.
Hydrocarbons with single bonds between the Carbons are called ALKANES.
Hydrocarbons with a double bond between one of the carbons are called ALKENES
Hydrocarbons with triple bonds between a pair of carbons are called ALKyNES
The rules
Each carbon atom must have 4 bonds. These bonds are shown as straight lines coming off the letter C - this C represents 1 carbon atom.
On the other end of each stick must be a C or a H ( for hydrogen atom)
Each H can only have 1 stick coming off it.
The Code
The prefix of a word indicates the number of carbon attoms.
meth = 1, eth = 2, prop = 3 but = 4, pent = 5, hex = 6, hept = 7, oct = 8, non = 9, dec = 10
eg propane = means 3 carbon atoms joined by a single bond between the carbons
eg heptane = means 7 carbon atoms joined by a single bond between the carbon atoms
eg butene = means 4 carbons one double bond between 2 of the carbons
Alcohols
The alcohols are not hydrocabons as they have oxygen added to them. We say an hydroxy group has been added to the end of a alkane (or other) chain. The hydroxy group is called the functional group and is denoted in the naming convention by the letters "ol"
eg ethanol = this means 2 carbons in the chain joined by single bonds with an OH group on the end.
Ways to make alcohols naturally include fermentation. We do this when we make beer or wine or whiskey.
There are some problems with making your own alcohol they include increasing the number of impurities in the brew that leads to a higher than required alcohol content or alcohols that are very poisonous.
Eg Methanol - very poisonous - sends you blind
Propanol - very poisonous dissolves cells.
Ethanol is the alcohol in drinks.
A note about fermentation
this is an organic reaction
Glucose -----> carbon dioxide + alcohol